What will be $\Delta S$ for the reaction: $2A + 3B \to 4C + 5D$ (in $J \ K^{-1}$)?
Given:
$\Delta S_A^o = 100 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_B^o = 120 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_C^o = 200 \ J \ mol^{-1} \ K^{-1}$
$\Delta S_D^o = 150 \ J \ mol^{-1} \ K^{-1}$

Standard entropies of $X_2, Y_2$ and $XY_5$ are $70, 50$ and $110 \ J \ K^{-1} \ mol^{-1}$ respectively. The temperature in Kelvin at which the reaction $\frac{1}{2} X_2 + \frac{5}{2} Y_2 \rightarrow XY_5$ with $\Delta H = -35 \ kJ \ mol^{-1}$ will be at equilibrium is . . . . . . (Nearest integer).

When $2 \ mol$ of an ideal gas $\left( C_{p,m} = \frac{5}{2} R \right)$ is heated from $300 \ K$ to $600 \ K$ at constant pressure,the change in entropy of the gas $\left( \Delta S \right)$ is:

Which one of the following has $\Delta S^o$ greater than zero?

Which of the following equations indicates an increase in entropy?

The standard entropies of $CO_{2(g)}$,$C_{(s)}$,and $O_{2(g)}$ are $213.5$,$5.740$,and $205 \ J \ K^{-1} \ mol^{-1}$ respectively. The standard entropy of formation of $CO_{2(g)}$ is $...... \ J \ K^{-1} \ mol^{-1}$.